Barium chloride

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Barium chloride
Barium chloride.jpg
Barium chloride crystals.
Names
IUPAC name
Barium chloride
Other names
Barium dichloride
Barium muriate
Muryate of Barytes
Identifiers
Jmol-3D images Image
Properties
BaCl2
Molar mass 208.23 g/mol (anhydrous)
244.26 g/mol (dihydrate)
Appearance White crystalline solid
Odor Odorless
Density 3.856 g/cm3 (anhydrous)
3.0979 g/cm3 (dihydrate)
Melting point 962 °C (1,764 °F; 1,235 K) (anhydrous)
Boiling point 1,560 °C (2,840 °F; 1,830 K)
31.2 g/100 mL (0 °C)
35.8 g/100 mL (20 °C)
59.4 g/100 mL (100 °C)
Solubility Soluble in methanol
Insoluble in ethanol, ethyl acetate, toluene
Vapor pressure ~0 mmHg
Thermochemistry
−858.56 kJ/mol
Hazards
Safety data sheet FisherScientific
Flash point Non-flammable
Lethal dose or concentration (LD, LC):
78 mg/kg (rat, oral)
50 mg/kg (guinea pig, oral)
Related compounds
Related compounds
 Magnesium chloride
Calcium chloride
Strontium chloride
Barium chlorate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Infobox references

Barium chloride is the inorganic compound with the formula BaCl2. It is a soluble barium compound, useful for the preparation of various barium compounds.

Properties

Chemical

Barium chloride reacts with sulfates to precipitate barium sulfate.

BaCl2 + SO4-2 → 2 Cl- + BaSO4

This reaction is used in identifying the sulfate species in a sample, though it also works with oxalates, phosphates or carbonates.

Reaction with sodium hydroxide gives barium hydroxide, which is moderately soluble in water.

BaCl2 + 2 NaOH → 2 NaCl + Ba(OH)2

Electrolysis of aq. barium chloride solutions will yield barium chlorate[1] and barium perchlorate[2], depending on the current densities.

Barium chloride dihydrate (BaCl2·2 H2O) is stable in the air at room temperature, but loses one water of crystallization above 55 °C, turning into the monohydrate form (BaCl2·H2O), and becomes anhydrous above 121 °C. The monohydrate form can also be obtained from its dihydrate by stirring it in methanol.[3]

Physical

Barium chloride is a white solid, soluble in water and methanol, but insoluble in ethanol and alkanes.

Availability

Barium chloride can be purchased online.

Preparation

Can be prepared by reacting barium carbonate with hydrochloric acid. The solution is concentrated by boiling it and is then left to cool, which causes the barium chloride to crystallize.

A good method of obtaining barium chloride from pottery-grade barium carbonate can be found here.

Projects

Handling

Safety

Barium chloride, like the other water-soluble barium salts, is highly toxic if ingested. A soluble sulfate salt, such as sodium sulfate or magnesium sulfate can be used as antidotes, as they convert the soluble barium ions to the insoluble barium sulfate, which is relatively non-toxic.

Storage

Barium chloride should be stored in closed bottles.

Disposal

Barium chloride should be mixed with sodium sulfate or magnesium sulfate before disposal.

Gallery

  • Barium chloride crystals on a watch glass

References

  1. ↑ http://www.chlorates.exrockets.com/barium.html
  2. ↑ http://www.chlorates.exrockets.com/ba_perk_prep.pdf
  3. ↑ Kirk-Othmer Encyclopedia of Chemical Technology. 3rd ed., Volumes 1-26. New York, NY: John Wiley and Sons, 1978-1984., p. V3: 469 (1978)

Relevant Sciencemadness threads

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